1 / 57

Writing Formulas!

Writing Formulas!. All compounds and molecules are neutral. Ions have charges. Bonding - a chemical attachment that forms a new substance. This new substance has new chemical and physical properties. Example: Sodium is an explosive metal. Chlorine is a toxic gas. Sodium chloride is salt.

katen
Download Presentation

Writing Formulas!

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Writing Formulas!

  2. All compounds and molecules are neutral. Ions have charges.

  3. Bonding - a chemical attachment that forms a new substance. This new substance has new chemical and physical properties Example: Sodium is an explosive metal.Chlorine is a toxic gas.Sodium chloride is salt.

  4. Metals • Tend to lose e- • Conductors • Malleable and ductile

  5. Nonmetals • Tend to gain e- • Non-conductors • Brittle

  6. Most common charges +1 +2 +3 ±4 -3 -2 -1 0 variable charges(always positive) +1 +2

  7. Remember… Opposites attract

  8. I. Bonds Ionic Bond- an exchange of electrons between a metal and a nonmetal. This creates oppositely charge ions that are attracted to each other.

  9. Gaining e- forms an anion (- ion) • Onions make you cry • Anions are negative • Losing e- forms a cation (+ ion) • Cats have paws • Cations are pawsitive

  10. I. Bonds B. Covalent Bonds - Formed by sharing electrons - Between two nonmetal atoms C. Metallic Bonds - Formed by a sea of electrons passing over the metal atoms - flexible connection, does not form a fixed molecule

  11. II. Compounds Compounds MUST be neutral A. Ionic Compounds - They only have two elements - the total amount of positive charge must equal the total amount of negative charge

  12. II. Compounds A. Ionic Compounds - subscripts are used to show how many of each element is needed to balance the overall charge

  13. II. Compounds A. Ionic Compounds - the metal's name does not change - the nonmetal retains the root of its name and adds the suffix -ide

  14. Sodium and Chlorine - + 11+ 17+ 11+ and 10- = 1+ Na+ 17+ and 18- = 1- Cl- NaCl sodium chloride

  15. Magnesium andOxygen 2+ 2- 12+ 8+ 12+ and 10- = 2+ Mg2+ 8+ and 10- = 2- O2- MgO magnesium oxide

  16. Magnesium and Chlorine - - 2+ 17+ 12+ 17+ 17+ and 18- = 1- Cl- 17+ and 18- = 1- Cl- 12+ and 10- = 2+ Mg2+ MgCl2 magnesium chloride

  17. What is the formula for Ionic Nomenclature sodium chloride What are the symbols and charges? Na +1 and Cl-1 How many of each atom is needed to make the compound neutral? NaCl

  18. What is the formula for Ionic Nomenclature sodium oxide What are the symbols and charges? Na +1 and O-2 How many of each atom is needed to make the compound neutral? Na2O

  19. What is the formula for Ionic Nomenclature aluminum chloride What are the symbols and charges? Al +3 and Cl-1 How many of each atom is needed to make the compound neutral? AlCl3

  20. What is the formula for Ionic Nomenclature aluminum oxide What are the symbols and charges? Al +3 and O -2 How many of each atom is needed to make the compound neutral? Al2O3

  21. II. Compounds A. Ionic Compounds - the formula of an ionic compound must be in the lowest whole number ratio of the two elements to form a neutral compound (empirical formula)

  22. What is the formula for Ionic Nomenclature magnesium oxide What are the symbols and charges? Mg +2 and O -2 How many of each atom is needed to make the compound neutral? MgO

  23. II. Compounds A. Ionic Compounds - metals with variable charges must include the charge in the name using Roman numerals

  24. What is the formula for Ionic Nomenclature lead (II) oxide What are the symbols and charges? Pb +2 and O -2 How many of each atom is needed to make the compound neutral? PbO

  25. What is the formula for Ionic Nomenclature manganese (IV) oxide What are the symbols and charges? Mn +4 and O -2 How many of each atom is needed to make the compound neutral? MnO2

  26. What is the formula for Ionic Nomenclature copper (II) nitride What are the symbols and charges? Cu +2 and N -3 How many of each atom is needed to make the compound neutral? Cu3N2

  27. II. Compounds A. Ionic Compounds 2. Polyatomic ion Compounds Polyatomic ions- a group of covalently bonded atoms with an overall charge that react as a group

  28. What is the formula for Ionic Nomenclature copper (II) sulfate What are the symbols and charges? Cu+2 and SO4-2 How many of each atom is needed to make the compound neutral? CuSO4

  29. What is the formula for Ionic Nomenclature sodium sulfate What are the symbols and charges? Na+1 and SO4-2 How many of each atom is needed to make the compound neutral? Na2 SO4

  30. II. Compounds A. Ionic Compounds 2. Polyatomic ion Compounds If more than one polyatomic ion is needed to make a neutral compound, you must use parenthesis to group the ion.

  31. What is the formula for Ionic Nomenclature barium hydroxide What are the symbols and charges? Ba+2 and OH -1 How many of each atom is needed to make the compound neutral? Ba(OH)2

  32. What is the formula for Ionic Nomenclature aluminum sulfate What are the symbols and charges? Al+3 and SO4-2 How many of each atom is needed to make the compound neutral? Al2 (SO4)3

  33. Nonmetals • Tend to gain e- • Nonconductor • Brittle

  34. II. Compounds B. Covalent (Molecular) Compounds Nonmetals want to gain electrons. When two nonmetals are together, they share the electrons.

  35. Hydrogen and Hydrogen H2 H H

  36. Nitrogen and Hydrogen (Ammonia) NH3 H H N H

  37. Hydrogen and Oxygen H2O O H H

  38. II. Compounds Naming covalent compounds - Because covalent compounds may form different compounds between two nonmetals with different ratios, the subscripts are denoted in the name by a prefix.

  39. 1 mono 2 di 3 tri 4 tetra 5 pent 6 hex 7 hept 8 oct 9 non 10 dec Covalent Nomenclature

  40. II. Compounds Naming covalent compounds - The element on the left will go first in the name. - The element on the right will go lastin the name. The root remains the same, but the suffix –ide is added. - The prefix in front of each element give the number of atoms (subscript written behind.)

  41. What is the formula for Covalent Nomenclature carbon monoxide 1 carbon 1 oxide CO

  42. What is the formula for Covalent Nomenclature carbon dioxide 1 carbon 2 oxide CO2

  43. What is the formula for Covalent Nomenclature diphosphorus pentoxide 2 phosphorus 5 oxide P2O5

  44. Is it covalent or ionic? Covalent - Look for prefixes (except dichromate) - 2 nonmetals - prefixes become subscripts - Remember these are the easy ones. No charges! No crisscross! Ionic - metal & nonmetal or metal & polyatomic - write the symbol and charge - balance charges to form a neutral compound (crisscross) - check to make sure you have the lowest whole number ratio!

  45. Write the formulas for these • lithium permanganate • tetraiodide monoxide • tin (II) oxide • tin (IV) oxide • diphosphorus pentoxide • aluminum dichromate • tetrasulfur hexaphosphide

  46. Write the names of the following: • KCl • Cl2O7 • CuSO3 • CO2 • CrN • NaNO3 • Sb2S3

  47. Write the formulas for these • nitrogen trioxide • magnesium cyanide • copper (II) hydroxide • carbon tetrafluoride • iron (III) bicarbonate • manganese (IV) chlorite • iron (III) carbonate

  48. Write the names of the following: • BaCl2 • CaSO4 • (NH4)2O • LiCN • Fe(OH)3 • Na3N • NiPO4

  49. Write the names of the following: • N2O • NO2 • PbO • PbO2 • Na2S • CBr4 • (NH4)2CO3

  50. II. Compounds C. Acids - (Special Ionic Compounds) 3. Acids- ionic compounds that start with H+1 plus an anion The anion changes its suffix: -ate converts to -ic acid -ite converts to -ous acid -ide converts to hydro--ic acid

More Related